Is the reaction of 8 grams of natural gas and 38 grams of oxygen gas to form 17 grams of carbon dioxide in 19 grams of water consistent with the law of conservation of mass?
Does 8 + 38 = 17 + 19 ?
To determine if the reaction is consistent with the law of conservation of mass, we need to calculate the total mass of the reactants and compare it with the total mass of the products.
Given:
Mass of natural gas (methane), CH4 = 8 grams
Mass of oxygen gas, O2 = 38 grams
Mass of carbon dioxide, CO2 = 17 grams
Mass of water, H2O = 19 grams
The balanced equation for the reaction is:
CH4 + 2O2 -> CO2 + 2H2O
Now, let's calculate the total mass of the reactants:
Total mass of reactants = mass of CH4 + mass of O2
= 8 grams + 38 grams
= 46 grams
Next, let's calculate the total mass of the products:
Total mass of products = mass of CO2 + mass of H2O
= 17 grams + 19 grams
= 36 grams
If the law of conservation of mass is to hold true, the total mass of the reactants should be equal to the total mass of the products.
Total mass of reactants = Total mass of products
46 grams = 36 grams
Since the total mass of the reactants (46 grams) doesn't equal the total mass of the products (36 grams), the reaction is not consistent with the law of conservation of mass.
To determine if the reaction is consistent with the law of conservation of mass, we need to calculate the total mass of the reactants and compare it to the total mass of the products.
Let's start by calculating the total mass of the reactants:
8 grams (natural gas) + 38 grams (oxygen gas) = 46 grams
Next, let's calculate the total mass of the products:
17 grams (carbon dioxide) + 19 grams (water) = 36 grams
By comparing the total mass of the reactants (46 grams) to the total mass of the products (36 grams), we can see that the mass of the products is less than the mass of the reactants. This result suggests that the reaction is not consistent with the law of conservation of mass.
In an isolated system, such as a chemical reaction, mass cannot be created or destroyed. According to the law of conservation of mass, the total mass of the reactants should be equal to the total mass of the products. In this case, it appears that there is a mass deficit.
Possible reasons for the mass deficit could include experimental errors in measurement or the presence of unaccounted-for products. It's important to double-check the calculations and ensure that all products and reactants are accounted for.